In a particular solution, acetic acid is 11% ionized at 25°C.
Calculate the pH of the...
In a particular solution, acetic acid is 11% ionized at 25°C.
Calculate the pH of the solution and the mass of acetic acid
(Ka=1.8x10^-5) dissolved to yield 1.00 L of solution.
1. Calculate the pH of the buffer of a solution of 0.02M acetic
acid (pKa = 4.76) and 0.04 M acetate
2. Based on your answer to the previous question, how much of a
0.5 M solution of HCl must be added to 200 mL of the above
mentioned solution to lower the pH to 2.50? Ignore volume
changes.
Calculate the pH and pOH of a
0.50 M solution of Acetic Acid. The Ka of HOAc is 1.8
x10-5
[H3O+]/(0.50-0.00095)=1.8x10-5 where did they get the .00095,
its said to take that as the second assumption
[H3O+]=9.4x10-4
[H3O+]/(0.50-0.00094)=1.85x10-5
[H3O+]=9.4x10-4 (this is said to be the third assumption)
Please, please help I really dont understand this, please show
all steps and be as descriptive as possible.
Calculate the pH at 25 C of a 0.75 M aqueous solution of
phosphoric acid (H3PO4). (Ka1, Ka2, and Ka3 for phosphoric acid are
7.5*10-3, 6.25*10-8, and
4.8*10-13, respectively.)
1. Calculate the pH at the equivalence point when a solution of
0.10M acetic acid is titrated with a solution of 0.10 M NaOH
solution. Given Ka for acetic acid is 1.8 x 10-5 .
2. The pH of blood serum is maintained by a proper balance of
H2CO3 and NaHCO3 concentrations. Calculate the volume of 5M NaHCO3
solution that should be mixed with a 10 mL of sample of blood which
is 2M in H2CO3 in order to maintain...
Calculate the pH at 25°C of a 0.65 M aqueous solution of oxalic
acid (H2C2O4). (Ka1 and Ka2 for oxalic acid are 6.5 × 10−2 and 6.1
× 10−5, respectively.